Iron can be protected from rusting by coating it in a thin layer of zinc in a process called galvanisation.The zinc layer is oxidised instead of the iron.Write out word equations for the oxidation reactions of both iron and zinc.

Iron:
Zinc:

Question

01-09-2021
Chemistry

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Iron can be protected from rusting by coating it in a thin layer of zinc in a process called galvanisation.The zinc layer is oxidised instead of the iron.Write out word equations for the oxidation reactions of both iron and zinc.

Iron:
Zinc:

Respuesta :

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devonwires devonwires · Answer 1 · 2021-09-01T19:26:01+02:00

Answer:

Rusting is an oxidation reaction. The iron reacts with water and oxygen to form hydrated iron (III) oxide, which we see as rust. Here is the word equation for the reaction: iron + water + oxygen → hydrated iron (III) oxide

In this reaction, zinc atoms each will lose two electrons (oxidation) and become Zn 2+ ions. The two electrons that are released by zinc will be gained by the Cu 2+ ions (reduction). The Cu2+ ions become Cu atoms. Total equation: Zn (s) + CuSO 4 (aq) --> Cu (s) + ZnSO 4 (aq)

Explanation:

Iron can be protected from rusting by coating it in a thin layer of zinc in a process called galvanisation.The zinc layer is oxidised instead of the iron.Write out word equations for the oxidation reactions of both iron and zinc. Iron: Zinc:

Respuesta :

Otras preguntas

Iron can be protected from rusting by coating it in a thin layer of zinc in a process called galvanisation.The zinc layer is oxidised instead of the iron.Write out word equations for the oxidation reactions of both iron and zinc.

Iron:
Zinc: